Mp4p3 Group 1

Can you come back to us?
Jen, Lenora, Linzi, and Alison


We all.........
-we have all been to the beach
-we all have beds
-we are all happy :)
-we all are girlssss !! :D
-we are all awesome
-we all love ice cream
-we all own a pair of jeans
-we all like to stalk people(only on weekends!)Linzi doesn't stalk people!! ... Jen just.. yeah.
6/8 Egg Drop Lab:

5/11 Alka Seltzer Lab:

Question: How will the mass of the reactants compare to the mass of the products when a gas is formed?
Hypothesis: The mass of the products will be less than that of the reactants when the gas is released.
IV: Mass of the reactants (grams)
DV: Mass of the products (grams)
Constants: The amount of water, the time you put the lid on when the lid is taken off
Procedure:

1. Measure the mass of the brown cylinder and cap.
2. Measure the mass of the alka seltzer and water with the brown cyclinder and cap, without letting the alka seltzer and water react.
3. Flip the alka seltzer into the jar with the cap and secure the lid.
4. Measure the mass while the cap is still on, and note any changes.
5. Remove cap, releasing gas, and measure the mass again.
6. Record results and note any changes in mass.
7. Complete 2 more trials.

AVERAGE DIFFERENCE: 3.15 grams

5/10 Lab:

Question: How will the mass of the reactants compare to the mass of the products in a reaction that produces a solid precipitate?
H: We think the mass of the products and reactants must be the same before and after the reaction according to the law of conservation of mass.
IV: Mass of the reactants (grams)
DV: Mass of the products (grams)
Constants: Same balance, mass of the glassware
Procedure:

1. Find the mass of the glassware.
2. Add some sodium iodide to test tube A.
3. Add some lead nitrate to test tube B.
4. Record new masses. (glass and chemicals)
5. Pick up the 2 test tubes and flip them upside down in the beaker.
6. Record the new mass. Subtract the glassware from the new mass to find the chemicals' mass.
7. Dump the chemicals into the funnel.
8. Do a second trial, and then a third trial, after cleaning the glassware thoroughly.
9. Record observations.

OBSERVATIONS:

• 1st trial: When the chemicals were dumped into the beaker together, they instantly changed to a bright, dark yellow.
• 2nd trial: Observations were very closely related to those of trial 1.
• 3rd trial: Observations were the same as the first and second trial.

4/27 Chemical Reaction Lab

Question: How will different chemicals react with each other when mixed?
Hypothesis: We think that the chemicals will dissolve into the solvents.
DV: Chemical dissolved (solute)
IV: The water/bromothmyl blue (solvent)
Constants: the amount of solvent, the amount of solute
Procedure:

1. Mix 1/2g of sodium bicarbonate in 10mL of bromothmyl blue.
2. Measure and record temperature.
3. Put 1/2g of sodium bicarbonate in 10 mL of water.
4. Measure and record temperature.
5. Mix 1/2g of calcium chloride in 10 mL of water.
6. Measure and record temperature.
7. Record observastions.

Substance Combination	Bromothymol Blue & Sodium bicarbonate	Sodium bicarbonate & water	Calcium Chloride & Water	Bromothmyl blue & Calcium Chloride	Calcium Chloride & Sodium bicarbonate
Beginning temperature (solvent)	21.6°C	21.1°C	21.8°C	21.4°C	21.5°C
Ending temperature (after solute is added)	19.5°C	19.5°C	27.1°	25°C	22.3°C

Observations:
Sodium bicarbonate & bromothmyl blue:
Not much happened, except that the bicarbonate dissolved.
Calcium Chloride & water:
After the sodium bicarbonate was added, the two substances seemed to fizz, almost like soda.
Sodium bicarbonate & water:
The sodium bicarbonate dissolved in the water.
**In the experiments the temperature lowered after the substance was added, except for the calcium chloride and water because the temperature raised almost 6 degrees.
Bromothmyl blue & Calcium Chloride:
When mixed it turned a light blue.
The temperature increased as it was mixed together.
Calcium Chloride & Sodium bicarbonate:
Temperature raised when mixed.
The mixture fizzed up for a few seconds almost like when you open a soda.

4/26: Substance Research!

Calcium chloride:

• solid at room temperature
• must be held in air tight containers
• used in ice control for roads
• can be produced from limestone
• recognized as safe by the Food and Drug Association

Sodium bicarbonate:

• used in baking soda
• common in medicine
• NaHCO3
• fine powder
• baking soda/bread soda

Bromothymol Blue:

• not a hazard to health, but could cause stomach aches or slight irriations
• used in measuring substances
• used in keeping the Ph in pools and in fish tanks
• recognized as safe and nutritious

4/18, Solubility & Temperature Lab:

Question: Does the temperature of the solvent affect the solubility of a mystery solute?

Hypothesis: We think that when the temperature of the solvent is high, the more soluble the solute will be, and vice versa.

Independent Variable: The temperature of the solvent (degrees Celsius)

Dependent Variable: The solubility (g/100mL)

Constants: The amount of water, the speed of stirring/mixing, the weighing paper, the mystery solute

Materials:

• Hot plate
• Beaker
• 10mL graduated cylinder
• Lab scoop
• Test tube
• Test tube rack
• Triple Beam Balance
• Temperature Sensor
• Mystery Substance

Procedure:

1. Measure the weighing paper
2. Measure 10 grams of "mystery substance"
3. Measure 10 mL of water
4. Heat a beaker of water on a hot plate.
5. Pour the mystery substance and water in a test tube and mix with a lap scoop.
6. Put the test tube in a the beaker of hot water and continue stirring.
7. Once the solute has completely dissolved in the solvent, set the test tube in the test tube rack.
8. Once a crystal is spotted in the test tube, take the temperature of the solution.

Here are our results!

Grams	10	8	6	4
First crystal seen at:	61.0 degrees	41.6 degrees	38.1 degrees	22.0 degrees

We plotted our points on the solubility graph and because of the way our points correspond to the one curve, we think that the mystery substance was potassium nitrate.

Concentration Lab!!! 4-12-11
Here is our lab:

Question= How doex mixing effect concentration?

Hypothesis= We think faster mixing will make the solution more concentrated.

Independent Variable= The solute and solvent

Depentdent Variable= The type of mixing process

Constants= Amount of water, amount of kool-aid, time spent mixing


Procedure=


1. Put 2g of kool-aid in 10mL of H2O in 4
2. Flick mix the 1st one for 30 seconds
3. Flip mix the 2nd for 30 seconds
4. Shake for 30 seconds
5. Leave the last one alone to dissolve by itself.

The concentration for each test tube was 1 g/5
mL!
To find it, we put the 2g over 10mL, then
simplified to get our final answer.
We mixed it by flicking it, flipping it, and shaking
it.
------> The "Hick mix" in the table is supposed to be Flick mix, but Alison messed up. :)

Watch our solubility vocab video! 4-11-11 :)

http://www.youtube.com/user/Team8Blue?
feature=mhum#p/u/0/nWt-B1BiwQM
The link is messed up, so just copy it and paste it into the search
bar.

Here are our materials!!!

1. Copper II Sulfate 5. Graduated Cylinder
2. Zinc Oxide 6. Test Tubes(4)
3. Lab Glasses 7. Test Tube Rack
4. Lab Scoop 8. Test Tube Stopper
9. Water































Solubility Lab 4-7-11
Heres what we did.......
1. First we added copper II sulfate to 5 mL of water. 2. Then we added copper II sulfate to 10 mL of water.
3. Next, we added zinc oxide to 5 mL of water.
4. Then we added zinc oxide to 10 mL of water.
5. Lastly, we mixed all of the substances by placing a stopper on top of the test tube and turning it back and forth.

Solubility Lab Set Up 4-6-11
Plan for lab tomorrow:
1. Put zinc oxide in 5 mL of water.
2. Put zinc oxide in 10 mL of water.
3. Put copper sulfate in 5 mL of water.
4. Put copper sulfate in 10 mL of water.
5. OBSERVE!!

Research!!!!
Zinc oxide:
http://en.wikipedia.org/wiki/Zinc_oxide#Safety

• non-toxic
• It is an additive in many products such as plastics, ceramics, glass, etc.
• It is very popular in medicine, such as in ointments!!

Copper II Sulfate:
http://msds.chem.ox.ac.uk/CO/copper_II_sulfate.html

• CuSO4
• Can be harmful if inhaled or ingested
• It is safe to work around if you are wearing safety glasses and have the proper ventilati